500.0 mL of hydrochloric acid 2.50M are mixed with 250.0mL of hydrochloric acid 3.75M. Assume that volumes are additive. What is the final concentration (in Molarity) of the hydrochloric acid?
500.0 mL of hydrochloric acid 2.50M are mixed with 250.0mL of hydrochloric acid 3.75M. Assume that...
A 65.0 mL sample of 0.513 M glucose (C6H12O6) solution is mixed with 160.0 mL of 2.33 M glucose solution. What is the concentration of the final solution? Assume the volumes are additive.
Sulfuric acid (250.0mL) is titrated with 176.5 mL 2.4 M NaOH to an equivalence point (the point where all the sulfuric acid is exactly neutralized). 2NaOH + H2SO4 -> 2H2O + Na2SO4 a) How many moles of Sulfuric acid were in the original 250.0 mL? moles of H2SO4 = b) What was the concentration of Sulfuric acid in the original 250.0 mL sample? Molarity of Sulfuric acid =
50. ml of a 1.0 M solution of hydrochloric acid, HCl, is titrated with a 1.0 M solution of sodium hydroxide. What is the pH after 51 mL of NaOH has been added? Assume that the volumes are additive.
50.0 mL of a stock solution of hydrochloric acid, HCl (aq), at 12.0 M is diluted by adding it to 150.0 mL of water, H2O. What is the concentration, in units of molarity, of the final, diluted solution?
4. If 50 liters of 12% hydrochloric acid (HCl) is mixed with 80 liters of 40% hydrochloric acid, how much acid would result and what would be the concentration of the final solution?
3 pts Question 13 What is the molarity of an aqueous solution of hydrochloric acid if 50.00 mL of 5.00 M HCl(aq) is diluted to a new volume of 100.0 mL? 5.00M 100M 2.50M 1.25M 3 pts Question 14 How many moles of sulfuric acid are in 300.0 mL of 2.00 M H2SO4(aq) 300 mol 0.300 ml 500 ml 0.600 mol
375 mL of a 0.150 M aqueous solution of silver (I) nitrate is mixed with 125 mL of a 0.125 M aqueous solution of sodium phosphate. Calculate the mass of precipitate that forms and the final concentration of each ion in the mixed solution. Volumes are additive and the precipitation reaction goes to completion. Can you show all work for calculating the final concentration of each ion in the reaction including Ag, NO3^-1, Na and PO4^-3
A 4.51 g sample of chalk is mixed with 23.8 mL of 3.0 M hydrochloric acid. It is filtered to obtain 3.64 g of calcium carbonate. What is the percent of calcium carbonate in the chalk?
2. A 25.0 mL sample of 0.12 M HBr is mixed with 15.0 mL of 0.10 M KOH. Calculate the pH of the mixture. Assume the volumes are additive.
A solution of 0.200 M KOH (17.6 mL) is mixed with 45.9 mL of 0.143 M HCl. Assuming that the final volume is the sum of the initial volumes, calculate: (a) the molarity of the K+ cation (b) the molarity of the Cl- anion (c) the pH of the final solution (d) the pOH of the final solution